Question

If 5.4 moles of Fe react with 4.7 moles of O2, what is the maximum amount of Fe2O3 (in moles) that can be produced? What is the limiting reactant?
a

3.1 moles of Fe2O3 is the maximum amount that can be produced. Oxygen is the limiting reactant.


b

2.7 moles of Fe2O3 is the maximum amount that can be produced. Iron is the limiting reactant.


c

7.1 moles of Fe2O3 is the maximum amount that can be produced. Oxygen is the limiting reactant.


d

10.8 moles of Fe2O3 is the maximum amount that can be produced. Iron is the limiting reactant.

Answer 1

Answer:

2.7 moles of Fe₂O₃ is the maximum amount that can be produced. Iron is the limiting reactant.

Explanation:

The balanced reaction is:

4 Fe + 3 O₂ → 2 Fe₂O₃

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of each compound participate in the reaction:

• Fe: 4 moles
• O₂: 3 moles
• Fe₂O3: 2 moles

The limiting reagent is one that is consumed first in its entirety, determining the amount of product in the reaction. When the limiting reagent is finished, the chemical reaction will stop.

You can use a simple rule of three as follows: if by stoichiometry 4 moles of Fe reacts with 3 moles of O₂, how much moles of Fe will be needed if 4.7 moles of O₂ react?

$moles of Fe =\frac{4. moles of Fe*4.7 moles of O_{2}}{3 moles of O_{2} }$

moles of O₂= 6.27

But 6.27 moles of Fe are not available, 5.4 moles are available. Since you have less moles than you need to react with 4.7 moles of O₂, iron Fe will be the limiting reagent.

So you can use a simple rule of three as follows: if by stoichiometry 4 moles of Fe produce 2 moles of Fe₂O₃, how many moles of Fe₂O₃ will be produced if 5.4 moles of Fe react?

$moles of Fe_{2}O_{3}=\frac{5.4 moles of Fe*2 moles of Fe_{2} O_{3} }{4 moles of Fe}$

moles of Fe₂O₃= 2.7 moles

Then:

2.7 moles of Fe₂O₃ is the maximum amount that can be produced. Iron is the limiting reactant.